What is the effect of increasing temperature on a reaction with ΔH > 0 and ΔS < 0?

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Q: What is the effect of increasing temperature on a reaction with ΔH > 0 and ΔS < 0?

Solution: For a reaction with ΔH > 0 and ΔS < 0, increasing temperature will make ΔG more positive, thus decreasing spontaneity.

Steps: 7

Step 1: Understand the terms ΔH and ΔS. ΔH > 0 means the reaction absorbs heat (endothermic), and ΔS < 0 means the disorder of the system decreases.
Step 2: Know that ΔG (Gibbs free energy) determines if a reaction is spontaneous. A negative ΔG means the reaction can happen on its own.
Step 3: The formula for ΔG is ΔG = ΔH - TΔS, where T is the temperature in Kelvin.
Step 4: Since ΔH is positive and ΔS is negative, TΔS will also be negative (because a negative number times a positive number is negative).
Step 5: As temperature (T) increases, the negative value of TΔS becomes more negative, making ΔG larger (more positive).
Step 6: A more positive ΔG means the reaction is less likely to happen spontaneously.
Step 7: Therefore, increasing temperature for a reaction with ΔH > 0 and ΔS < 0 decreases its spontaneity.